2. Cyanate ion in waste solutions from gold-mining operations can be destroyed by treatment with hypochlorite ion in basic solution. Write a balanced oxidation-reduction equation for this reaction. OCN (aq) + OCT (aq) + OH(aq)CO₂ (aq) + N₂(g) + Cr(aq) + H₂O(1) (Hint: Notice that in the oxidation half-reaction, OCN yields two products.)

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2. Cyanate ion in waste solutions from gold-mining operations can be destroyed by treatment
with hypochlorite ion in basic solution. Write a balanced oxidation-reduction equation for this
reaction.
OCN (aq) + OCT(aq) + OH(aq)CO₂ (aq) + N₂(g) + Cr(aq) + H₂O(1)
(Hint: Notice that in the oxidation half-reaction, OCN yields two products.)
Transcribed Image Text:2. Cyanate ion in waste solutions from gold-mining operations can be destroyed by treatment with hypochlorite ion in basic solution. Write a balanced oxidation-reduction equation for this reaction. OCN (aq) + OCT(aq) + OH(aq)CO₂ (aq) + N₂(g) + Cr(aq) + H₂O(1) (Hint: Notice that in the oxidation half-reaction, OCN yields two products.)
Balancing Oxidation-Reduction Reactions using Method of Half Reactions
Reactions Occur in acid
1. Assign oxidation numbers to determine what is oxidized and what
is reduced.
2. Write the oxidation and reduction
half-reactions.
3. Balance each half-reaction.
1. Balance elements other than H and O.
2. Balance O by adding H₂O.
3. Balance H by adding H".
4. Balance charge by adding electrons
4. Multiply the half-reactions by integers so that the electrons gained and lost are the same.
5. Add the half-reactions, subtracting things that appear on both sides.
6. Make sure the equation is balanced according to mass.
7. Make sure the equation is balanced according to charge.
Reaction Occurs in Base
8. If a reaction occurs in a basic solution, one can balance it as if it occurred.
in acid.
9. Once the equation is balanced, add OH to each side to "neutralize" the H' in the equation an
create water in its place.
10. If this produces water on both sides,
you might have to subtract water from each side.
Transcribed Image Text:Balancing Oxidation-Reduction Reactions using Method of Half Reactions Reactions Occur in acid 1. Assign oxidation numbers to determine what is oxidized and what is reduced. 2. Write the oxidation and reduction half-reactions. 3. Balance each half-reaction. 1. Balance elements other than H and O. 2. Balance O by adding H₂O. 3. Balance H by adding H". 4. Balance charge by adding electrons 4. Multiply the half-reactions by integers so that the electrons gained and lost are the same. 5. Add the half-reactions, subtracting things that appear on both sides. 6. Make sure the equation is balanced according to mass. 7. Make sure the equation is balanced according to charge. Reaction Occurs in Base 8. If a reaction occurs in a basic solution, one can balance it as if it occurred. in acid. 9. Once the equation is balanced, add OH to each side to "neutralize" the H' in the equation an create water in its place. 10. If this produces water on both sides, you might have to subtract water from each side.
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